MendeleviumElectron Configuration, Bohr Model, Valence Electrons & Orbital Diagram

The electron configuration of Mendelevium is written as 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 5f¹³ 7s². Applying the Aufbau principle — filling orbitals from lowest to highest energy — plus the Pauli Exclusion Principle and Hund's Rule, we systematically place all 101 electrons: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 5f¹³ 7s². Mendelevium fills f-orbitals — seven orbitals accommodating up to 14 electrons — that are energetically shielded by outer s and d electrons, which explains why lanthanide and actinide elements have such similar surface chemistry despite differing nuclear charges.

Mendelevium follows the standard Aufbau filling order without exception. The noble gas shorthand [Rn] 5f¹³ 7s² replaces the inner-shell electrons with the symbol of the preceding noble gas, highlighting that only the outer electrons — 5f¹³ 7s² — are chemically active. Note: for Period 4+ elements, the 4s orbital fills before 3d per Madelung's rule, even though 3d ends at a lower energy in the final atom.

Shell-by-shell, Mendelevium's 101 electrons are distributed as: K-shell (n=1): 2 electrons; L-shell (n=2): 8 electrons; M-shell (n=3): 18 electrons; N-shell (n=4): 32 electrons; O-shell (n=5): 31 electrons; P-shell (n=6): 8 electrons; Q-shell (n=7): 2 electrons. The Q-shell (n=7) is the valence shell, containing 3 electrons.

Chemically, this configuration places Mendelevium in Group 3 with oxidation states of 3, 2. This configuration directly predicts Mendelevium's bonding mode, reactivity toward oxidizing and reducing agents, and the stoichiometry of its most common compounds.

The SPDF orbital model describes Mendelevium's electrons not as planetary orbits but as three-dimensional probability clouds — each orbital a region of space where an electron is most likely to be found. Mendelevium's 101 electrons occupy 17 distinct subshells: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 5f¹³ 7s², governed by three quantum mechanical rules.

The Pauli Exclusion Principle ensures no two electrons in Mendelevium share the same four quantum numbers (n, l, m_l, m_s). This is why the 1s orbital holds only 2 electrons, the full p-subshell holds 6, d holds 10, and f holds 14. Without this rule, all 101 electrons would collapse into the 1s orbital. In Mendelevium, Hund's Rule applies to seven f-orbitals — each occupied singly before pairing. The energetic near-degeneracy of 4f/5d/6s (or 5f/6d/7s) orbitals means minor perturbations determine the exact filling order, causing the configurational complexity of f-block elements.

Following standard orbital filling, Mendelevium fills orbitals in the sequence: 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p. The final electron enters the 7s² subshell, making Mendelevium a f-block element with 3 valence electrons in Group 3.

The outermost electrons — 7s² — are Mendelevium's chemical agents. Understanding the 7s² occupancy — how many electrons, whether paired or unpaired, the orbital shape involved — is the foundation for predicting Mendelevium's bonding geometry, oxidation behavior, and compound formation.

Mendelevium's chemical reactivity is shaped by three interlocking properties: electronegativity (1.3 Pauling), first ionization energy (6.58 eV), and electron affinity (0 eV). Its electronegativity is low-to-moderate (1.3) — predominantly metallic character, electropositive tendency. Mendelevium donates electrons to partners rather than accepting them — the hallmark of electropositive metals.

The first ionization energy of 6.58 eV is relatively low, confirming Mendelevium's readiness to lose electrons — a quintessentially metallic trait.

In standard chemical conditions, Mendelevium forms predominantly +3 oxidation state compounds, consistent with its 3 valence electrons and f-block character.

Placing Mendelevium between Fermium (Z=100) and Nobelium (Z=102) reveals the incremental property changes that make the periodic table a predictive tool.

Fermium → Mendelevium: adding one proton and one electron increases nuclear charge by 1. Valence electrons remain at 3 — both occupy Group 3. Electronegativity: 1.3 → 1.3 | Ionization energy: 6.5 → 6.58 eV. Atomic radius increases from 190 pm to 190 pm, consistent with descending a group with additional shells.

Mendelevium → Nobelium: the additional proton and electron in Nobelium maintains 3 valence electrons but shifts subshell occupancy. Both elements share Actinide character, with Nobelium exhibiting slightly different electronegativity. These comparisons confirm that Mendelevium sits at a well-defined chemical inflection point in the periodic table.